If the bond order is zero, the molecule cannot form. The higher bond orders indicate greater stability for the new molecule.
For a more in-depth look, check the periodic table to see what kind of bonding you’ve got going on. [5] X Expert Source Chris Hasegawa, PhDRetired Science Professor & Dean Expert Interview. 29 July 2021.
Depending on the size and complexity of a particular atom, it might have only one orbital, or it might have as many as four. When the nearest orbital shell is full, new electrons start to gather in the next orbital shell out from the nucleus, and continue until that shell is also full. The collection of electrons continues in ever-widening orbital shells, as larger atoms have more electrons than smaller atoms. [6] X Research source
The Lewis dot structure for diatomic nitrogen would be N≡N. Each nitrogen atom features one electron pair and three unbonded electrons. When two nitrogen atoms meet, their combined six unbonded electrons intermingle into a powerful triple covalent bond. [8] X Research source
The Lewis dot structure for diatomic nitrogen would be N≡N. Each nitrogen atom features one electron pair and three unbonded electrons. When two nitrogen atoms meet, their combined six unbonded electrons intermingle into a powerful triple covalent bond. [8] X Research source
Bonding electrons: By noting how full the orbital shells of each atom are, you can determine how many of the electrons in higher energy states will be able to fill the more stable, lower-energy-state shells of the corresponding atom. These “filling electrons” are referred to as bonding electrons. Antibonding electrons: When the two atoms try to form a molecule by sharing electrons, some electrons will actually be driven to higher-energy-state orbital shells as the lower-energy-state orbital shells are filled up. These electrons are referred to as antibonding electrons. [11] X Research source
